{"id":155987,"date":"2024-10-16T18:48:45","date_gmt":"2024-10-16T18:48:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=155987"},"modified":"2024-10-16T18:48:47","modified_gmt":"2024-10-16T18:48:47","slug":"the-formula-for-sodium-phosphate","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/16\/the-formula-for-sodium-phosphate\/","title":{"rendered":"The formula for sodium phosphate"},"content":{"rendered":"\n<p>The formula for sodium phosphate: <\/p>\n\n\n\n<p>A. NaPO\u2084<\/p>\n\n\n\n<p>B. Na(PO4)3 <\/p>\n\n\n\n<p>C. Na\u2083PO\u2084.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct formula for sodium phosphate is<strong> C<\/strong>. <strong>Na\u2083PO\u2084<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation<\/h3>\n\n\n\n<p>Sodium phosphate is a chemical compound composed of sodium ions and phosphate ions. The phosphate ion (PO\u2084\u00b3\u207b) carries a -3 charge, meaning it can bond with three sodium ions (Na\u207a), each of which has a +1 charge. This stoichiometric relationship is critical in determining the correct chemical formula for the compound.<\/p>\n\n\n\n<p>To break it down further:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Ionic Charges<\/strong>: The phosphate ion has a charge of -3, while the sodium ion has a charge of +1. Therefore, to balance the overall charge of the compound to zero (as required for stable ionic compounds), we need three sodium ions to neutralize one phosphate ion:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(3 \\times (+1) + (-3) = 0)<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Combining the Ions<\/strong>: Given the need for three sodium ions to balance one phosphate ion, the formula becomes Na\u2083PO\u2084. This indicates that for every one phosphate ion, there are three sodium ions.<\/li>\n\n\n\n<li><strong>Common Usage<\/strong>: Sodium phosphate is commonly used in various applications, including food processing, as a buffering agent in laboratory settings, and in pharmaceuticals. It is available in various forms, such as monosodium phosphate (NaH\u2082PO\u2084) and disodium phosphate (Na\u2082HPO\u2084), each differing by the number of sodium ions and their resultant properties and uses.<\/li>\n\n\n\n<li><strong>Molecular Weight<\/strong>: The molecular weight of sodium phosphate can be calculated as follows:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na): 22.99 g\/mol (3 \u00d7 22.99 g\/mol = 68.97 g\/mol)<\/li>\n\n\n\n<li>Phosphorus (P): 30.97 g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 16.00 g\/mol (4 \u00d7 16.00 g\/mol = 64.00 g\/mol)<\/li>\n\n\n\n<li>Total molecular weight of Na\u2083PO\u2084 = 68.97 g\/mol + 30.97 g\/mol + 64.00 g\/mol = 163.94 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>In summary, Na\u2083PO\u2084 accurately represents sodium phosphate, reflecting its composition of three sodium ions and one phosphate ion, establishing its importance in chemistry and various industries.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The formula for sodium phosphate: A. NaPO\u2084 B. Na(PO4)3 C. Na\u2083PO\u2084. The Correct Answer and Explanation is: The correct formula for sodium phosphate is C. Na\u2083PO\u2084. Explanation Sodium phosphate is a chemical compound composed of sodium ions and phosphate ions. The phosphate ion (PO\u2084\u00b3\u207b) carries a -3 charge, meaning it can bond with three sodium [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-155987","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155987","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=155987"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155987\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=155987"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=155987"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=155987"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}